Find the enthalpy of neutralisation in $kJ/mol$ for the reaction between $NH_4OH$ and $HCN$ in aqueous solution,given that the enthalpies of ionisation of $NH_4OH$ and $HCN$ are $7 \ kJ/mol$ and $8 \ kJ/mol$ respectively,and the enthalpy of neutralisation of a strong acid and a strong base is $-57.3 \ kJ/mol$.

At $1 \ atm$ pressure,$\Delta S = 75 \ J/K \cdot mol$ and $\Delta H = 30 \ kJ/mol$. The temperature of the reaction at equilibrium is $....... \ K$.

The energy of combustion per mole of $H_2$,$LPG$,and octane follows the order:

For which of the following processes will the value of $\Delta H^{\circ} - \Delta G^{\circ}$ be approximately zero?

Find the enthalpy of neutralisation of $NH_4OH$ and $HCN$ in aqueous solution if the enthalpy of ionisation of $NH_4OH$ and $HCN$ are $7 \ kJ/mol$ and $8 \ kJ/mol$ respectively. Also,the enthalpy of neutralisation of $H^{+}$ and $OH^{-}$ is $-57.3 \ kJ/mol$.

$A$ system consisting of $1 \, mole$ of an ideal gas undergoes a reversible process,$A$ $\rightarrow B$ $\rightarrow C$ $\rightarrow A$ (schematically indicated in the figure below). If the temperature at the starting point $A$ is $300 \, K$ and the work done in the process $B \rightarrow C$ is $1 \, L \, atm$,the heat exchanged in the entire process in $L \, atm$ is $....$